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MasteringChemistry: Chapter 5 Homework Secure https://session.masteringchemistry.com/myct/itemView?assignmentProblemID-95531982&offset-next; Chapter 5 Homework Exercise 5.80 K) 10 Constants I Periodic Table Part A Carbon monoxide gas reacts with hydrogen gas to form methanol. CO(g) + 2H2 (g)-CH3OH(g) A 1.95 L reaction vessel, initially at 305 K contains carbon monoxide gas at a partial pressure of 232 mmHg and hydrogen gas at a partial pressure of 388 mmHg Identify the limiting reactant and determine the theoretical yield of methanol in grams. Express your answer with the appropriate units. Value Units Submit Request Answer

Explanation / Answer

V   = 1.95L

T   = 305K

PCO = 232mmHg   = 232/760   = 0.3053atm

PV = nRT

n    = PV/RT

       = 0.3053*1.95/0.0821*305    = 0.024moles

no of moles of CO = 0.024 moles

V   = 1.95L

T   = 305K

PH2 = 388mmHg   = 388/760   = 0.51atm

PV = nRT

n    = PV/RT

       = 0.51*1.95/0.0821*305    = 0.0397moles

no of moles of H2   = 0.0397 moles

CO(g) + 2H2(g) ----------> CH3OH(g)

1 moles of CO react with 2 moles of H2

0.024 moles of CO react with = 2*0.024/1   = 0.048 moles of H2

H2 is limiting reactant

2 moles of H2 react with CO to gives 1 mole of CH3OH

0.0397 moles of H2 react with CO to gives = 1*0.0397/2   = 0.01985moles of CH3OH

mass of CH3OH = no of moles * gram molar mass

                            = 0.01985*32    = 0.6352 g

theoretical yiled of CH3OH   = 0.6352g

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